Laws of Chemical Combination Last Updated : 02 Apr, 2024 Comments Improve Suggest changes Like Article Like Report Laws of Chemical Combination are one of the most fundamental building blocks of the subject of chemistry. As in our surrounding different matter reacts with each other and form various kind of different substances. Laws of Chemical Combination are the collection of laws that explains how these substances combine together to form anything at all. When matter reacts with another matter, a chemical reaction happens which changes the form, properties, or characteristics of the matter drastically. This interaction of matter with each other is governed by the Laws of Chemical Combination. What is Law of Chemical CombinationA collection of laws that governs the interaction; such as how they combined to form other matter, of matter with each other, is combinedly called the Laws of Chemical Combinations. The law of chemical combination collection includes five laws, which are as follows: Laws of Conservation of MassLaws of Definite ProportionsLaws of Multiple ProportionsGay-Lussac's Law of Gaseous VolumesAvogadro's LawLaw of Conservation of MassLaw of Conservation of Mass states that "Mass can neither be created nor can be destroyed in a chemical reaction" but it can be transformed from one form to another. In other words, in an enclosed system whenever matter undergoes a chemical or physical change, the total mass of reacting matter (reactants or matter before the change) is exactly equal to the total mass of reaction products. As no products or reactants are allowed to exit the system in a closed system, there is no loss of the substance, and hence the mass is conserved. For example, in automobiles, fuel is burned to create energy for vehicles to move forward and the fuel is converted into fumes such as carbon dioxide, carbon monoxide, or sulfur dioxide, etc. This law was first outlined by Mikhail Lomonosov in 1756 and then further refinements are proposed by Antoine Lavoisier in 1773 after a lot of experiments. Example of Law of Conservation of MassFor an example of conservation of mass, let's consider the formation of a water molecule from oxygen and hydrogen molecules. Balance chemical Reaction of formation of water is: 2H2 + O2 → 2H2O In the above example, 2 molecules of Hydrogen combine with 1 molecule of Oxygen to form 2 molecules of water. Mass of H is 1 unit and O is 16 units. Mass of 2 molecules of Hydrogen (2H2) is 4 units.Mass of 1 molecule of Oxygen (O2) is 32 units.Mass of 2 molecules of water (2H2O) is 36 units.2H2 + O2 → 2H2O 4 unit 32 unit 36 unit The total mass of the reactants equals the total mass of the products in this case. Furthermore, the number of hydrogen and oxygen atoms in the reactant and product sides are also equal. Law of Definite ProportionsLaw of Definite Proportions which is also known as the Law of Constant Composition, states that in any given chemical compound the composition of the element by mass is always remains the same. In other words, this means that the ratio of the mass of the elements in the chemical compounds always remains the same i.e., in a water molecule there will always be two hydrogens and one oxygen molecule. The law of Definite proportion is first proposed by Joseph Louis Proust in the late 18th century and many scholars have proved it since then. This law helps us identify between different chemical compounds as well. Example of Law of Definite Proportions Consider the different molecules of Oxides of Nitrogen for examples of the law of definite proportions. In the above example of oxides of Nitrogen if we take any amount of Oxygen and Nitrogen in the sample then the ratio of nitrogen to oxygen in the formed NO will always be 1:1. Similarly, the ratio of nitrogen to oxygen for NO2, N2O, and N2O2 will be 1:2, 2:1 and 2:2 respectively. This is guaranteed by the law of definite proportions. Law of Multiple ProportionsAccording to the Law of Multiple Proportions, If two elements combined to form more than one compound under different circumstances, then the ratio of the masses for one element when second mass is fixed for all different compounds is always a small whole number. The Law of Multiple Proportions is also known as Dalton's Law, as it was first proposed by Dalton in the year 1804. This law doesn't hold for non-stoichiometric compounds as well as heavy molecules such as polymers and oligomers. Example of Law of Multiple ProportionsCarbon and oxygen combine to form two distinct compounds (under different circumstances). The first is the most common gas, CO2 (Carbon dioxide), and the second is CO (Carbon monoxide). Lets take 12 grams of carbon, and by the calculation of moles we can find that it reacts with 16 grams of Oxygen to make Carbon Monoxide and with 32 grams of oxygen to form Carbon dioxide. As a result, the ratio of mass of oxygen in the first and second compounds is 2:1 = 32/16 = 2, (whole number). Gay Lussac’s Law of Gaseous VolumesGay Lussac enacted this law based on his observations in 1808. This law states that "when gases are produced or combined in a chemical reaction, they do so in a simple volume ratio provided that all the gases are at the same temperature and pressure." This law is regarded as an of definite proportions for gases and the difference between these two chemical combination laws is that Gay Lussac's Law is stated the ratio of volume, whereas the law of definite proportions is stated in terms of mass. Example of Gay Lussac’s Law of Gaseous VolumesIn the above example 2 volumes of H2 combines 1 volume of O2 to form 2 volumes of H2O. H2 (g) + O2 (g) → 2H2O (g) Avogadro’s LawAccording to Avogadro’s Law, an ‘equal volume of all gases contains the equal number of molecules under the same conditions of temperature and pressure.' This law was proposed In 1811 by none other than Avogadro himself. In other words, this law states that the volume and number of moles of any gas are always directly proportional to each other. This means that two liters of hydrogen have the same number of molecules as two liters of oxygen at the same temperature and pressure. Example of Avogadro’s LawEquivalent volumes of different gases contain the same number of molecules at the same temperature and pressure. In the above example CL2 and H₂ has 1 volume each combines to form 2 volume of HCL. Here, Mole is a unit of measurement for substance. 1 mole substance contains 6.02214076×10²³ particles. Read More, Gas LawsMole ConceptChemical Bonding Comment More infoAdvertise with us Next Article Dalton's Atomic Theory N naimishsahu08 Follow Improve Article Tags : School Learning Class 9 Chemistry Chemistry-Class-9 Chemistry-Concepts +1 More Similar Reads Chemistry Chemistry is the scientific study of matter, its properties, composition, and interactions. It is often referred to as the central science because it connects and bridges the physical sciences, such as physics and biology. Understanding chemistry is crucial for comprehending the world around us, fro 6 min read Chapter 1 - Some Basic Concepts of ChemistryImportance of Chemistry in Everyday LifeImportance of Chemistry in Everyday Life: The scientific study of matter's properties and behavior is known as chemistry. 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